We are asked to calculate the percent ionization of a 0.15 M formic acid solution in a solution containing 0.11 M potassium formate.
Recall that the percent ionization is given by:
Remember that weak acids partially dissociate in water and that acids donate H+ to the base (water in this case).
The dissociation of formic acid is as follows:
HCOOH(aq) + H2O(l)⇌ H3O+(aq) + HCOO–(aq)
It has a Ka value of 1.8x10-4 that can be found from a textbook or the internet.
Calculate the percent ionization of a 0.15 M formic acid solution in a solution containing 0.11 M potassium formate.
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